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I II III IV V
Chemical Reactions
III. Types of Chemical Reactions
A. Combustion
CH4(g) + 2O2(g) CO2(g) + 2H2O(g)
the burning of any substance in O2 to produce heat
A + O2 B
Na(s)+ O2(g)
C3H8(g)+ O2(g) 5 3 4
A. Combustion
Products: contain oxygen hydrocarbons form CO2 + H2O
CO2(g)+ H2O(g)
Na2O(s) 4 2
B. Synthesis
the combination of 2 or more substances to form a compound
only one product
A + B AB
B. Synthesis
H2(g) + Cl2(g) 2 HCl(g)
Al(s)+ Cl2(g) AlCl3(s)2 3 2
B. Synthesis
Products: ionic - cancel charges covalent - hard to tell
C. Decomposition
a compound breaks down into 2 or more simpler substances
only one reactant
AB A + B
C. Decomposition
2 H2O(l) 2 H2(g) + O2(g)
KBr(l) K(s) + Br2(l) 2 2
C. Decomposition
Products: binary - break into elements others - hard to tell
D. Single Replacement
one element replaces another in a compound metal replaces metal (+) nonmetal replaces nonmetal (-)
A + BC B + AC
D. Single Replacement
Cu(s) + 2AgNO3(aq) Cu(NO3)2(aq) + 2Ag(s)
Fe(s)+ CuSO4(aq) Cu(s)+ FeSO4(aq)
D. Single Replacement
Products: metal metal (+) nonmetal nonmetal (-) free element must be more active (check activity series)
Br2(l)+ NaCl(aq) N.R.
AB + CD AD + CB
E. Double Replacement
ions in two compounds “change partners” cation of one compound combines with
anion of the other
E. Double Replacement
Pb(NO3)2(aq) + K2CrO4(aq) PbCrO4(s) + 2KNO3(aq)
Pb(NO3)2(aq)+ KI(aq) PbI2(s)+ KNO3(aq)
E. Double Replacement
Products: switch negative ions one product must be insoluble (check
solubility table)
NaNO3(aq)+ KI(aq) N.R.
2 2